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AP Chemistry Chapter 5 and 19 Jeopardy

AP Chemistry Chapter 5 and 19 Jeopardy. Jennie L. Borders. Round 1 – Chapter 5. Round 2 – Chapter 19. Click to go to Round 2. Energy 100.

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AP Chemistry Chapter 5 and 19 Jeopardy

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  1. AP ChemistryChapter 5 and 19 Jeopardy Jennie L. Borders

  2. Round 1 – Chapter 5

  3. Round 2 – Chapter 19 Click to go to Round 2

  4. Energy 100 Calculate the DE for a process in which the system releases 57.5kJ of heat while doing 22.5kJ of work on the surroundings. Is the process endothermic or exothermic? -80kJ exothermic

  5. Energy 200 Calculate the DE for a process in which the system absorbs 105kJ of heat from its surroundings while doing 29kJ of work on the surroundings. Is the process exothermic or endothermic? 76kJ endothermic

  6. Energy 300 If two positive particles are brought closer together, then explain what would happen to the electrostatic potential energy and why. Eel = kQ1Q2 If both particles are d positively charged, then Q1 and Q2 are positive making the value of Eel positive. As distance decreases, the magnitude of Eel increases, so it is not a favorable process.

  7. Energy 400 Calculate the kinetic energy in joules of a 45g golf ball moving at 61 m/s. 84J

  8. Energy 500 What is the kinetic energy of an 850 lb. motorcycle moving at 66 mph? (1 kg = 2.2047 lb. 1 mi = 1.6093 km) 1.7 x 105J

  9. Stoichiometry 100 Calculate the DH for the production of 0.200 mol of AgCl by the following reaction: Ag+(aq) + Cl-(aq) AgCl(s) DH = -65.5kJ -13.1kJ

  10. Stoichiometry 200 For this reaction, DH for the formation of 0.632mol of O2. 2KClO3(s) 2KCl(s) + 3O2(g) DH = -89.4kJ -18.8kJ

  11. Stoichiometry 300 Calculate the amount of heat transferred when 2.4g of Mg reacts at constant pressure. 2Mg(s) + O2(g) 2MgO DH = -1204kJ -59kJ

  12. Stoichiometry 400 Calculate the amount of heat transferred when 45.0g of CH3OH is decomposed by the following reaction at constant pressure. CH3OH(g) CO2(g) + 2H2(g) DH = 90.7kJ 128kJ

  13. Stoichiometry 500 Calculate the amount of heat transferred for the formation of 6.32g O2. CH3OH(l) + 3/2O2(g) CO2(g) +2H2O(l) DH = -726.5kJ 95.66kJ

  14. q = mCDT 100 Two solid objects, A and B, are placed in boiling water and allowed to come to temperature there. Each is then lifted out and placed in separate beakers containing 1000g of water at 10.0oC. Object A increases the water temperature by 3.50oC; B increases water temperature by 2.60oC. Which object has the larger heat capacity and what extra piece of information do you need to figure out which has the higher specific heat capacity? Object A; mass of each object.

  15. q = mCDT 200 How many kJ of heat are needed to raise the temperature of 10.00kg of liquid water from 24.6oC to 46.2oC? 904kJ

  16. q = mCDT 300 The specific heat of iron metal is 0.450 J/gK. How many J of heat are necessary to raise the temperature of a 1.05kg block of iron from 25.0oC and 88.5oC? 3.00 x 104 J

  17. q = mCDT 400 The specific heat of ethylene glycol is 2.42 J/gK. How many J of heat are needed to raise the temperature of 62.0g of ethylene glycol from 13.1oC to 40.5oC? 4.11 x 103 J

  18. q = mCDT 500 What is the molar heat capacity of water? 75.31 J/moloC

  19. DH 100 Calculate the DH for 3H2(g) + O3(g) 3H2O(g) using the following information: 2H2(g) + O2(g)  2H2O(g)DH = -483.6 kJ 3O2(g)  2O3(g)DH = 284.6 kJ -867.7kJ

  20. DH 200 Calculate the DH for C2H4(g) + 6F2(g) 2CF4(g) + 4HF(g) using the following information: H2(g) + F2(g)  2HF(g)DH = -537kJ C(s) + 2F2(g)  CF4(g) DH = -680kJ 2C(s) + 2H2(g)  C2H4(g)DH = 523kJ -2486.3kJ

  21. DH 300 Calculate the DH for N2O(g) + NO2(g) 3NO(g) using the following information: N2(g) + O2(g)  2NO(g)DH = 180.7kJ 2NO(g) + O2(g)  2NO2(g)DH = -113.1kJ 2N2O(g)  2N2(g) + O2(g)DH = -163.2kJ 155.65kJ

  22. DH 400 Calculate the DH for the following reaction using information from Appendix C. SiCl4(l) + 2H2O(l) SiO2(s) + 4HCl(g) -68.34kJ

  23. DH 500 When C10H8(s) is combusted it yeilds CO2(g), H2O(l), and 5154 kJ/mol. What is the standard enthalpy of formation for C10H8. 75.68kJ

  24. Definitions 100 What is the internal energy of a system? Total kinetic and potential energy

  25. Definitions 200 What is a closed system? A system in which heat can be transferred between the system and the surroundings but not mass.

  26. Definitions 300 What is a state function? A property that only depends on the initial and final states, not on the path taken.

  27. Definitions 400 For a given process at constant pressure, DH is negative. Is the process exothermic or endothermic? exothermic

  28. Definitions 500 By what means can the internal energy of a closed system increase? Increase in heat of the system or work done on the system.

  29. Calorimetry 100 A 2.200g sample of C6H4O2 is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/oC. The temperature of the calorimeter increases from 23.44oC to 30.57oC. What is the heat of combustion per mole of C6H4O2? -2740.2 kJ/mol

  30. Calorimetry 200 A 1.800g sample of C6H5OH was burned in a bomb calorimeter whose total heat capacity is 11.66kJ/oC. The temperature of the calorimeter plus contents increased from 21.36oC to 26.37oC. What is the heat of combustion per mole of C6H5OH? -3074.74kJ

  31. Calorimetry 300 A 2.500g sample of glucose is burned in a bomb calorimeter. The heat of combustion of glucose is -15.57kJ/mol. The temperature of the calorimeter increases from 20.55oC to 23.25oC. What is the total heat capacity of the calorimeter? 14.42 kJ/oC

  32. Calorimetry 400 What a 9.55g sample of solid NaOH dissolves in 100.0g of water in a coffee-cup calorimeter, the temperature rises from 23.6oC to 47.4oC. Calculate DH in kJ/mol of NaOH for the solution process. -45.61 kJ/mol

  33. Calorimetry 500 When a 3.88g sample of solid NH4NO3 dissolves in 60.0g of water in a coffee-cup calorimeter, the temperature drops from 23.0oC to 18.4oC. Calculate DH in kJ/mol of NH4NO3 for the solution process. 25.36 kJ/mol

  34. Definitions 200 What is a spontaneous process? A spontaneous process is one that proceeds on its own without any assistance.

  35. Definitions 400 What is a reversible process? In a reversible process, a system is changed in such a way that the system and surroundings can be restored to their original state by exactly reversing the change. (DOES NOT EXIST)

  36. Definitions 600 What is entropy? Entropy is the measure of the randomness, disorder, or dispersal of energy in a system.

  37. Definitions 800 What is the difference in translational, vibrational, and rotational energy? Translational motion is the movement of an entire molecule. Vibrational motion is the stretching and bending of bonds. Rotational energy is the spinning of a molecule.

  38. Definitions 1000 What are the 3 laws of thermodynamics? 1st Law = Energy is conserved. 2nd Law = Any irreversible process results in an increase in entropy. 3rd Law = The entropy of a pure crystalline solid is 0 at 0K.

  39. Spontaneous Processes 200 Consider the vaporization of liquid water to steam at a pressure of 1atm. In what temperature range is it a spontaneous process? Temperatures higher than 100oC.

  40. Spontaneous Processes 400 Does the change in DE depend on the particular pathway taken to carry out a change of state? No, it is a state function.

  41. Spontaneous Processes 600 Consider what happens when TNT explodes. Determine the sign for q, w, and DE. Explosions are combustion reactions so q is negative since it is exothermic. w is also negative because the reactants will expand to form products. Since q and w are negative, DE will also be negative.

  42. Spontaneous Processes 800 Is the following process spontaneous, nonspontaneous, or at equilibrium? The formation of CH4 and O2 molecules from CO2 and H2O. Nonspontaneous – It would be spontaneous in the reverse direction because it would be combustion.

  43. Spontaneous Processes 1000 Is the following process spontaneous, nonspontaneous, or at equilibrium? Ice melting at 0oC equilibrium

  44. Entropy 200 Predict the sign of DS as the reaction proceeds to the right. BCl3(g) + NH3(g) Cl3BNH3(s) negative

  45. Entropy 400 Which of the following reactions would have a –DS? • 2Fe2O3(s) 4Fe(s) + 3O2(g) • Mg+2(aq) + 2OH-(aq)  Mg(OH)2(s) • H2(g) + C2H4(g)  C2H6(g) 2 and 3

  46. Entropy 600 Which reaction involves the largest decrease in entropy? • 2CO(g) + O2(g) 2CO2(g) • Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq) • 4La(s) + 3O2(g)  2La2O3(s) 3

  47. Entropy 800 Which of the following reactions has the largest +DS value per mole of Cl2? • 2NH4Cl(s)N2(g) + 4H2(g) + Cl2(g) • Cl2(g)  2Cl(g) • H2(g) + Cl2(g)  2HCl(g) 1

  48. Entropy 1000 For the reaction Cl2(g) + 3F2(g) 2ClF3(g) the DHof is -163.2 kJ/mol and the DGof is -123kJ/mol for ClF3. Calculate the DSo in J/K for the reaction at 298K. -269.8 J/K

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